The recommended daily sugar intake is 50.0 gram. How many moles of sugar (C12H22O11) are in 50.0 grams of sugar?

Compare how mammals care for their young with the other groups of animals.

slega [8]

Well, even though some baby mammals are born different ways, they all drink milk that comes from their mothers' bodies. Baby pigs, dolphins, bats and elephants all drink milk! Because the babies rely on their mother's milk to live, the mammalmommies have to care for their young.

4 0

2 years ago

Now balance the chemical reaction by providing the correct whole number coefficients:

Tcecarenko [31]

Answer:

2(C4H10)+13(O2)->8(CO2)+[](H20)

Explanation:

sorry i couldn’t get the last one

7 0

3 years ago

Read 2 more answers

Ammonia (NH3) ionizes according to the following reaction: NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH–(aq) The base dissociation constant

Ira Lisetskai [31]

Answer:

pH = 9.6

Explanation:

According to Brönsted-Lowry theory, NH₃ is a base and NH₄⁺ its conjugate acid. When they are together in a solution, the form a buffer, which is used to resist abrupt changes in pH when an acid or a base is added. pOH fro a buffer can be found using Henderson-Hasselbalch equation.

$pOH = pKb + log\frac{conjugateacid}{base}$

Since NH₄Cl is a strong electrolyte, [NH₄Cl] = [NH₄⁺]

$pOH = pKb + log\frac{[NH_{4}^{+} ]}{[NH_{3}]} =4.7+log\frac{0.035M}{0.070M} =4.4$

Now, we can find pH using the following expression:

pH + pOH = 14

pH = 14 - pOH = 14 - 4.4 = 9.6

7 0

3 years ago

The enthalpy of reaction changes somewhat with temperature. Suppose we wish to calculate ΔH for a reaction at a temperature T th

Contact [7]

Answer:

-99.8 kJ

Explanation:

We are given the methodology to answer this question, which is basically Kirchhoff law . We just need to find the heats of formation for the reactants and products and perform the calculations.

The standard heat of reaction is

ΔrHº = ∑ ν x ΔfHº products - ∑ ν x ΔfHº reactants

where ν are the stoichiometric coefficients in the balanced equation, and ΔfHº are the heats of formation at their standard states.

Compound ΔfHº (kJmol⁻¹)

SO₂ -296.8

O₂ 0

SO₃ -395.8

The balanced chemical equation is

SO₂(g) + ½O₂(g) → SO₃(g)

Thus

Δr, 298K Hº( kJmol⁻¹ ) = 1 x (-395.8) - 1 x (-296.8) = -99.0 kJmol⁻¹

Now the heat capacity of reaction will be be given in a similar fashion:

Cp rxn = ∑ ν x Cp of products - ∑ ν x Cp of reactants

where ν is as above the stoichiometric coefficient in the balanced chemical equation.

Cprxn ( JK⁻¹mol⁻¹) = 50.7 - ( 39.9 + 1/2 x 29.4 ) = - 3.90

= -3.90 JK⁻¹mol⁻¹

Finally Δr,500 K Hº = Δr, 298K Hº + CprxnΔT

Δr,500 K Hº = - 99 x 10³ J + (-3.90) JK⁻¹ ( 500 - 298 ) K = -99,787.8

= -99,787.8 J x 1 kJ/1000 J = -99.8 kJ

Notice thie difference is relatively small that is why in some problems it is o.k to assume the change in enthalpy is constant over a temperature range, especially if it is a small range of temperatures.

3 0

3 years ago

The following reaction was performed in a sealed vessel at 772 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at

Paladinen [302]

Answer: The value of $K_c$ for the given equation is 160.2